1. Chapter 5 Section 1: Organizing the Elements Key Concepts:
How did Mendeleev organize the elements in his periodic table?
What evidence helped verify the usefulness of Mendeleev’s table?

2. Question 1:
Describe how Mendeleev organized the elements into rows and columns in his periodic table.
Answer: Mendeleev arranged the elements in rows in order of increasing mass so that elements with similar properties were in the same column.

3. Question 2:
How did the discovery of new elements such as gallium demonstrate the usefulness of Mendeleev’s table?
Answer: The close match between Mendeleev’s predictions and the actual properties of new elements showed how useful his periodic table could be.

4. Question 3:
Scientists before Mendeleev had proposed ways to organize the elements. Why were Mendeleev’s efforts more successful?
Answer: Mendeleev provided an organizing principle that worked for all off the known elements.

5. Question 4:
What characteristic of solitaire did Mendeleev use as a model for his periodic table?
Answer: In solitaire, cards are arranged into categories called suits and ordered by value.

6. Question 5: Why did Mendeleev leave spaces in his table?
Answer: In order to place elements with similar properties in the same column, Mendeleev needed to leave spaces for undiscovered elements.

7. Question 6:
In general, how can a scientist test the correctness of a scientific model?
Answer: The scientist tests weather the model can be used to make accurate predictions.

8. Question 7:
Explain why it would not have been possible for a scientist in 1750 to develop a table like Mendeleev’s.
Answer: With only 17 known elements to work with, the scientist would not have had enough data.

9. Question 8:
How was Mendeleev able to predict the properties of elements that had not yet been discovered?
Answer: Mendeleev based his predictions on the properties of nearby elements and other elements in the same column.

10. Chapter 5 Section 2: The Modern Periodic Table Key Concepts:
How is the modern periodic table organized?
What does the atomic mass of an element depend on?
What categories are used to classify elements on the periodic table?
How do properties vary across a period in the periodic table?

11. Question 1:
What determines the order of the elements in the modern periodic table?
Answer: In the modern periodic table, elements are arranged by increasing atomic number.

12. Question 2: Describe the periodic law.
Answer: Properties of elements repeat in a predictable way when atomic numbers are used to arrange elements into groups.

13. Question 3: What two factors determine the atomic mass of an element?
Answer: Atomic mass is a value that depends on the distribution of an element’s isotopes in nature and the masses of those isotopes.

14. Question 4:
Name three categories that are used to classify the elements in the periodic table.
Answer: Metals, nonmetals, and metalloids.

15. Question 5:
What major change occurs as your move from left to right across the periodic table?
Answer: The elements become less metallic and more nonmetallic in their properties.

16. Question 6:
The atomic mass of iodine (I) is less than the atomic mass of tellurium (Te). But an iodine atom has one more proton than a tellurium atom. Explain how this situation is possible.
Answer: Answers may include that the tellurium isotopes that are most abundant have many neutrons in their nuclei or that all tellurium atoms have more neutrons than iodine atoms.

17. Question 7:
Explain how you know that no new element with an atomic number less than 100 will be discovered.
Answer: The atomic number of an element corresponds to the number of protons in the element’s atoms. The atomic number must be a whole number. All the places between 1 and 100 are already filled with existing elements.

18. Question 8:
Compare the reactions with water of the elements sodium and magnesium.
Answer: Sodium reacts quickly and violently with water at room temperature. Magnesium will not react unless the water is hot.

19. Chapter 5 Section 3: Representative Groups Key Concepts:
Why do the elements in a group have similar properties?
What are some properties of the A groups in the periodic table?

20. Question 1: Explain why elements in a group have similar properties.
Answer: They have similar properties because they have the same number of valence electrons.

21. Question 2:
What is the relationship between an alkali metal’s location in Group 1A and its reactivity?
Answer: The reactivity of alkali metals increases from the top of Group 1A to the bottom.

22. Question 3: What element exists in almost every compound in your body?
Answer: Carbon

23. Question 4: Which Group 5A elements are found in fertilizer?
Answer: Nitrogen and phosphorus.

24. Question 5: Which group of elements are found in fertilizer?
Answer: The noble gases (Group 8A)

25. Question 6: Why is hydrogen located in a group with reactive metals?
Answer: Hydrogen is placed with other elements that have a single valence electron.

26. Question 7: What biological function requires magnesium?
Answer: The process that uses sunlight to produce sugar in plants.

27. Question 8: Why is aluminum recycled?
Answer: The energy needed to purify recycled aluminum is only about 5% of the energy needed to extract aluminum from bauxite.

28. Question 9: What is the main use of sulfur?
Answer: To produce sulfuric acid.

29. Question 10: Why is chlorine added to drinking water?
Answer: Chlorine is added to drinking water to kill bacteria.

30. Question 11:
In which class of elements is there a greater range of properties, the metals or the nonmetals? Give an example to support your answer.
Answer: Accept all answers that are supported by reasonable arguments. Students may choose nonmetals and say that they display a greater range of physical properties and reactivity.

31. Question 12:
What happens to the reactivity of nonmetals within a group from the top of the group to the bottom?
Answer: The reactivity of nonmetals decrease from the top to the bottom of a group.